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SYLLABUS

Chapter-1

Atomic structure 1.1 Sub - atomic particles 1.2 Atomic models - Rutherford’s nuclear model of atom 1.3 Developments to the Bohr’s model of atom 1.4 Bohr’s model for hydrogen atom 1.5 Quantum mechanical considerations of subatomic particles 1.6 Quantum mechanical model of an atom. Important features of quantum mechanical model of atom-orbitals and quantum numbers-shapes of atomic orbitals-energies of orbitals-filling of orbitals in atoms. Aufbau principle, Pauli’s exclusion principle and Hund’s rule of maximum multiplicityElectronic configurations of atoms-Stability of half filled and completely filled orbitals.

Chapter-2

classification of elements and periodicity in properties 2.1 Need to classify elements 2.2 Genesis of periodic classification 2.3 Modern periodic law and present form of the periodic table 2.4 Nomenclature of elements with atomic number greater than 100 2.5 Electronic configuration of elements and the periodic table 2.6 Electronic configuration and types of elements s, p, d and f blocks 2.7 Trends in physical properties-periodic trends in chemical properties-periodic trends and chemical reactivity.

Chapter-3

Chemical bonding and molecular structure 3.1 Kossel-Lewis approach to chemical bonding 3.2 Ionic or electrovalent bond 3.3 Bond Parameters 3.4 The Valence Shell Electron Pair Repulsion (VSEPR) theory, 3.5 Valence bond theory 3.6 Hybridisation 3.7 Coordinate bond 3.8 Molecular orbital theory-bonding in some homonuclear diatomic molecules 3.9 Hydrogen bonding.

Chapter-4

states of matter: gases and liquids 4.1 Intermolecular forces 4.2 Thermal energy 4.3 Intermolecular forces Vs Thermal interactions 4.4 The gaseous state 4.5 The gas laws 4.6 Ideal gas equation 4.7 Graham’s law of diffusion - Dalton’s law of partial pressures 4.8 Kinetic molecular theory of gases 4.9 Kinetic gas equation of an ideal gas (no derivation)- Deduction of gas laws from kinetic gas equation 4.10 Distribution of molecular speeds - rms, average and most probable speeds - kinetic energy of gas molecules 4.11 Behaviour of real gases - deviation from ideal gas behaviour-compressibility factor Vs pressure diagrams of real gases 4.12 Liquefaction of gases 4.13 Liquid state - properties of liquids in terms of inter molecular interactions - vapour pressure, viscosity and surface tension (Qualitative ideal only, no mathematical derivation).

Chapter-5

stoichiometry 5.1 Some basic concepts 5.2 Laws of chemical combinations, Gay Lussac’s law of gaseous volumes, Dalton’s atomic theory, Avogadro law 5.3 Atomic and molecular masses - mole concept and molar mass concept of equivalent weight, 5.4 Percentage composition of compounds and calculations of empirical and molecular formulae of compounds 5.5 Stoichiometry and stoichiometric calculations 5.6 Methods of expressing concentrations of solutions 5.7 Redox reactions 5.8 Oxidation number concept 5.9 Types of redox reactions 5.10 Balancing of redox reactions-oxidation number method-half reaction (ion-electron) method 5.11 Redox reactions in titrimetry.

Chapter-6

Thermodynamics 6.1 Thermodynamic terms 6.2 Applications-work-enthalpy-extensive and intensive properties-heat capacity 6.3 Measurement of “U and H”: Calorimetry 6.4 Enthalpy change, 'Dr H’ of reactions 6.5 Enthalpies for different types of reactions 6.6 Spontaneity 6.7 Gibbs Energy change and equilibrium 6.8 Absolute entropy and the third law of thermodynamics.

Chapter-7

chemical equilibrium and acids - bases 7.1 Equilibrium in physical process 7.2 Equilibrium in chemical process - dynamic equilibrium 7.3 Law of chemical equilibrium - law of mass action and equilibrium constant 7.4 Homogeneous equilibria, equilibrium constant in gaseous systems, relationship between Kp and Kc 7.5 Heterogeneous equilibria 7.6 Applications of equilibrium constant 7.7 Relationship between equilibrium constnat ‘K’, reaction Quotient ‘Q’ and Gibbs energy ‘G’ 7.8 Factors affecting equilibria, -Le-chatelier’s principle application to industrial synthesis of ammonia and sulphur trioxide 7.9 Ionic equilibrium in solutions, 7.10 Acids, bases and salts - Arrhenius, BronstedLowry and Lewis concepts of acids and bases 7.11 Ionisation of acids and bases 7.12 Buffer solutions 7.13 Solubility equilibria of sparingly soluble salts - solubility product constant-common ion effect on solubility of Ionic salts.

Chapter-8

hydrogen and its compounds 8.1 Position of hydrogen in the periodic table 8.2 Dihydrogen-occurance and isotopes 8.3 Preparation of dihydrogen 8.4 Properties of dihydrogen 8.5 Hydrides: Ionic, covalent, and nonstiochiometric hydrides 8.6 Water: Physical properties: structure of water, ice, chemical properties of water; hard and soft water; hard and soft water temporary an